Nomenclature PO4

3-

phosphate ion

C2H3O2-

acetate ion

HC2H3O2

Acetic Acid

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CHEMICAL BONDS A chemical bond is an electrostatic

(attractive) force that holds oppositely

charged particles together in an ionic

compound.

Bonds are represented using lines.

FORMS OF CHEMICAL BONDS

There are 3 forms bonding atoms:

Ionic—complete transfer of 1 or more electrons from one atom to another (one loses, the other gains) between a metal and a nonmetal.

Covalent—some valence electrons shared between atoms of nonmetals.

Metallic – holds atoms of a metal together

Most bonds are

somewhere in

between ionic

and covalent.

PROPERTIES OF COMPOUNDS Ionic Compounds- high melting and boiling points due to

strong bonds between ions. Ionic compounds in an aqueous

(water) solution conduct an electric charge, this means they

are good conductors of electricity. They gain or lose

electrons.

Covalent Compounds- low melting and boiling points and

have weak bonds. They only share electrons.

Metallic Compounds- have a “sea of electrons”, metal

atoms do not share or lose their valence electrons with

neighboring atoms. Instead they overlap their electrons.

They are malleable, ductile, and good conductors of

electricity. They tend to have high melting and boiling

points.

COMMON NAMES A lot of chemicals have common

names as well as the proper

IUPAC name. (International Union

of Pure and Applied Chemistry)

Chemicals that should always be

named by common name and

never named by the IUPAC

method are: H2O water, not dihydrogen monoxide

NH3 ammonia, not nitrogen trihydride

CATION +

ANION --->

COMPOUND

A neutral compound

requires

equal number of +

and - charges.

COMPOUNDS FORMED FROM IONS

Na+ + Cl- --> NaCl

Predicting Charges on Monatomic Ions KNOW THESE !!!!

+1 +2 -3 -2 -1 0

Cd+2

PROPERTIES OF IONIC COMPOUNDS

FORMING NACL FROM NA AND CL2

A metal atom can

transfer an electron to

a nonmetal.

The resulting cation

and anion are

attracted to each

other by

electrostatic forces.

IONIC COMPOUNDS

NH4+

Cl-

ammonium chloride, NH4Cl

SOME IONIC COMPOUNDS

Mg2+ + N-3 ---->

Mg3N2

magnesium nitride

Sn4+ + O2- ---->

SnO2

Tin (IV) oxide

calcium fluoride

Ca2+ + 2 F- ---> CaF2

FORMULAS OF IONIC COMPOUNDS

Formulas of ionic compounds are determined

from the charges on the ions

atoms ions

–

Na + F : Na+ : F : NaF

sodium + fluorine sodium fluoride formula

Charge balance: 1+ 1- = 0

MONATOMIC IONS

WRITING A FORMULA

Write the formula for the ionic compound that will form

between Ba2+ and Cl.

Solution:

1. Balance charge with + and – ions

2. Write the positive ion of metal first, and the

negative ion Ba2+ Cl

Cl

3. Write the number of ions needed as

subscripts BaCl2

4. Keep all subscripts together for polyatomic ions

(ex: CO3-2) K+ + CO3

-2 → K2CO3

NH4+ + CO3

-2 → (NH4)2CO3

LEARNING CHECK

Write the correct formula for the compounds containing the following ions:

1. Na+, S2-

a) NaS b) Na2S c) NaS2

2. Al3+, Cl-

a) AlCl3 b) AlCl c) Al3Cl

3. Mg2+, N3-

a) MgN b) Mg2N3 c) Mg3N2

SOLUTION

1. Na+, S2-

b) Na2S

2. Al3+, Cl-

a) AlCl3

3. Mg2+, N3-

c) Mg3N2

COMMON POLYATOMIC IONS Negative 1 Charge

Acetate C2H3O2-1

Perchlorate ClO4-1

Chlorate ClO3-1

Chlorite ClO2-1

Hypochlorite ClO-1

Cyanide CN-1

Hydrogen Carbonate or

Bicarbonate HCO3-1

Hydrogen Sulfate HSO4-1

Hydroxide OH-1

Nitrate NO3-1

Permanganate MnO4-1

Nitrite NO2-1

Negative 2 Charge

Carbonate CO3-2

Chromate CrO4-2

Dichromate Cr2O7-2

Oxalate C2O4-2

Sulfate SO4-2

Sulfite SO3-2

Selenate SeO4-2

Negative 3 Charge

Phosphate PO4-3

Phosphite PO3-3

Borate BO3-3

Positive 1 Charge

Ammonium NH4+1

CRISS CROSS METHOD

• Positive Ion always

written first

• If you have a

polyatomic ion, you

must put it in

parentheses ( ) if

you cross a number

other than 1 to the

bottom. Ex: Be+2

SO4-3 Be3(SO4)2

You do not have to

put Be in

parentheses since it

is a monatomic ion

(just one atom).

COUNTING ATOMS

NaCl

NaOH

Mg(OH)2

Ca3(PO4)2

NH4Cl

(NH4)3PO4

LiNO3

BeSO4

SrSO3

Cs2CO3

How many atoms are in the following compounds?

NAMING COMPOUNDS

1. Cation first, then anion

2. Monatomic cation = name of the

element

Ca2+ = calcium ion

3. Monatomic anion = root + -ide

Cl = chloride

CaCl2 = calcium chloride

Binary Ionic Compounds:

NAMING BINARY IONIC COMPOUNDS

Examples:

NaCl

ZnI2

Al2O3

sodium chloride

zinc iodide

aluminum oxide

LEARNING CHECK

Complete the names of the following binary compounds:

Na3N sodium ________________

KBr potassium ________________

Al2O3 aluminum ________________

MgS _________________________

TRANSITION METALS

Elements that can have more than one possible

charge MUST have a Roman Numeral to indicate

the charge on the individual ion.

1+ or 2+ 2+ or 3+

Cu+, Cu2+ Fe2+, Fe3+

copper(I) ion iron(II) ion

copper (II) ion iron(III) ion

NAMES OF VARIABLE IONS

These elements REQUIRE Roman Numerals because they can have more than one possible charge:

anything except Group 1A, 2A, Ag, Zn, Cd, and Al (You should already know the charges on these!) Or another way to say it is: Transition metals and the metals in groups 4A and

5A (except Ag, Zn, Cd, and Al) require a Roman Numeral.

FeCl3 (Fe3+) iron (III) chloride

CuCl (Cu+ ) copper (I) chloride

SnF4 (Sn4+) tin (IV) fluoride

PbCl2 (Pb2+) lead (II) chloride

Fe2S3 (Fe3+) iron (III) sulfide

EXAMPLES OF OLDER NAMES OF

CATIONS FORMED FROM TRANSITION

METALS (YOU DO NOT HAVE TO MEMORIZE THESE)

LEARNING CHECK

Complete the names of the following binary

compounds with variable metal ions:

FeBr2 iron (_____) bromide

CuCl copper (_____) chloride

SnO2 ___(_____ ) ______________

Fe2O3 ________________________

Hg2S ________________________

NAMING COMPOUNDS

Poly- many

Bi- 2

Polyatomic ions- many (2 or more) atoms bonded

together that have a charge (positive or negative

charge).

Binary-2 atoms or elements bonded together

Ternary- 3 or more atoms bonded together

Oxidation number- charge of the atom

NAMING IONIC COMPOUNDS

POLYATOMIC IONS NO3

-

nitrate ion

NO2-

nitrite ion

POLYATOMIC IONS

You can make additional polyatomic ions by adding a H+ to the ion!

CO3 -2 is carbonate

HCO3– is hydrogen carbonate

H2PO4– is dihydrogen phosphate

HSO4– is hydrogen sulfate

TERNARY IONIC NOMENCLATURE

Writing Formulas

Write each ion, cation first. Don’t show charges in the final formula.

Overall charge must equal zero. If charges cancel, just write symbols. If not, use subscripts to balance charges.

Use parentheses to show more than one of a particular polyatomic ion.

Use Roman numerals indicate the ion’s charge when needed (stock system)

TERNARY IONIC NOMENCLATURE

Sodium Sulfate

Na+ and SO4 -2

Na2SO4

Iron (III) hydroxide

Fe+3 and OH-

Fe(OH)3

Ammonium carbonate

NH4+ and CO3

–2

(NH4)2CO3

TYPES OF REACTIONS Endothermic reaction- a chemical reaction in which a

greater amount of energy is required to break the bonds

than is released. (energy in) These reactions are cool to the

touch in a container.

Exothermic reaction- a chemical reaction in which more

energy is released than is required to break the bonds.

(energy out) The formation of ionic compounds is

exothermic. Burning something releases energy and is an

exothermic reaction.

Delocalized electron- the electrons involved in metallic

bonding that are free to move easily from one atom to the

next.

Oxyanion- a polyatomic ion composed of an element,

usually a nonmetal, bonded to one or more oxygen atoms. Ex: Sulfate SO4

-2 Sulfite SO3-2 Nitrate NO3

- , Nitrite NO2- , etc.

Formula unit- the simplest ratio of ions represented in an

ionic compound. Ex: Ba2O2 can be simplified to BaO,

Ca2(SO4)2 can be simplified to CaSO4

LEARNING CHECK

1. aluminum nitrate

a) AlNO3 b) Al(NO)3 c) Al(NO3)3

2. copper(II) nitrate

a) CuNO3 b) Cu(NO3)2 c) Cu2(NO3)

3. Iron (III) hydroxide

a) FeOH b) Fe3OH c) Fe(OH)3

4. Tin(IV) hydroxide

a) Sn(OH)4 b) Sn(OH)2 c) Sn4(OH)

NAMING TERNARY COMPOUNDS

Contains at least 3 elements

There MUST be at least one polyatomic ion

(it helps to circle the ions)

Examples:

NaNO3 Sodium nitrate

K2SO4 Potassium sulfate

Al(HCO3)3 Aluminum bicarbonate

or

Aluminum hydrogen carbonate

LEARNING CHECK

Match each set with the correct name:

1. Na2CO3 a) magnesium sulfite

MgSO3 b) magnesium sulfate

MgSO4 c) sodium carbonate

2 . Ca(HCO3)2 a) calcium carbonate

CaCO3 b) calcium phosphate

Ca3(PO4)2 c) calcium bicarbonate

MIXED PRACTICE!

Name the following:

1. Na2O

2. CaCO3

3. PbS2

4. Sn3N2

5. Cu3PO4

6. HgF2

MIXED UP… THE OTHER WAY

Write the formula:

1. Copper (II) chlorate

2. Calcium nitride

3. Aluminum carbonate

4. Potassium bromide

5. Barium fluoride

6. Cesium hydroxide

NAMING MOLECULAR COMPOUNDS

CH4 methane BCl3

boron trichloride

CO2 Carbon dioxide

All molecular/

covalent

compounds

formed from

two or more

nonmetals.

Ionic

compounds

generally

involve a metal

and nonmetal

(NaCl)

MOLECULAR (COVALENT) NOMENCLATURE

FOR TWO NONMETALS

Prefix System (binary compounds)

1. Less electronegative atom

comes first.

2. Add prefixes to indicate # of atoms. Omit mono-

prefix on the FIRST element. Mono- is OPTIONAL on

the SECOND element (in this class, it’s NOT

optional!).

3. Change the ending of the

second element to -ide.

MOLECULAR NOMENCLATURE PREFIXES

PREFIX

mono-

di-

tri-

tetra-

penta-

hexa-

hepta-

octa-

nona-

deca-

NUMBER

1

2

3

4

5

6

7

8

9

10

• CCl4

• N2O

• SF6

• carbon tetrachloride

• dinitrogen monoxide

• sulfur hexafluoride

MOLECULAR NOMENCLATURE:

EXAMPLES

• arsenic trichloride

• dinitrogen pentoxide

• tetraphosphorus decoxide

• AsCl3

• N2O5

• P4O10

MORE MOLECULAR EXAMPLES

LEARNING CHECK

Fill in the blanks to complete the following

names of covalent compounds.

CO carbon ______oxide

CO2 carbon _______________

PCl3 phosphorus _______chloride

CCl4 carbon ________chloride

N2O _____nitrogen _____oxide

LEARNING CHECK

1. P2O5

a) phosphorus oxide

b) phosphorus pentoxide

c) diphosphorus pentoxide 2. Cl2O7

a) dichlorine heptoxide

b) dichlorine oxide

c) chlorine heptoxide 3. Cl2 a) chlorine

b) dichlorine

c) dichloride

OVERALL STRATEGY FOR NAMING

CHEMICAL COMPOUNDS.

A FLOW CHART FOR NAMING BINARY COMPOUNDS.

MIXED REVIEW

Name the following compounds:

1. CaO

a) calcium oxide b) calcium(I) oxide

c) calcium (II) oxide

2. SnCl4

a) tin tetrachloride b) tin(II) chloride

c) tin(IV) chloride

3. N2O3

a) nitrogen oxide b) dinitrogen trioxide c) nitrogen trioxide

SOLUTION

Name the following compounds:

1. CaO

2. SnCl4

3. N2O3

a) calcium oxide

c) tin(IV) chloride

b) Dinitrogen trioxide

MIXED PRACTICE

1. Dinitrogen monoxide

2. Potassium sulfide

3. Copper (II) nitrate

4. Dichlorine heptoxide

5. Chromium (III) sulfate

6. Iron (III) sulfite

7. Calcium oxide

8. Barium carbonate

9. Iodine monochloride

MIXED PRACTICE

1. BaI2

2. P4S3

3. Ca(OH)2

4. FeCO3

5. Na2Cr2O7

6. I2O5

7. Cu(ClO4)2

8. CS2

9. B2Cl4

ACID NOMENCLATURE

Acids

Compounds that form H+ in water.

Formulas usually begin with ‘H’.

In order to be an acid instead of a gas, binary acids

must be aqueous (dissolved in water)

Ternary acids are ALL aqueous

Examples:

HCl (aq) – hydrochloric acid

HNO3 – nitric acid

H2SO4 – sulfuric acid

Anion Ending Acid Name

-ide hydro-(stem)-ic acid

-ate (stem)-ic acid

-ite (stem)-ous acid

ACID NOMENCLATURE REVIEW

No Oxygen

w/Oxygen

An easy way to remember which goes with which…

“In the cafeteria, you ATE something ICky”

ACID NOMENCLATURE FLOWCHART

hydro- prefix

-ic ending

2 elements

-ate ending

becomes

-ic ending

-ite ending

becomes

-ous ending

no hydro- prefix

3 elements

ACIDSstart with 'H'

• HBr (aq)

• H2CO3

• H2SO3

• 2 elements, -ide

• 3 elements, -ate

• 3 elements, -ite

hydrobromic acid

carbonic acid

sulfurous acid

ACID NOMENCLATURE

• hydrofluoric acid

• sulfuric acid

• nitrous acid

• 2 elements

• 3 elements, -ic

• 3 elements, -ous

HF (aq)

H2SO4

HNO2

ACID NOMENCLATURE

H+ F-

H+ SO42-

H+ NO2-

NAME ‘EM!

HI (aq)

HCl

H2SO3

HNO3

H3PO4

WRITE THE FORMULA!

Hydrobromic acid

Nitrous acid

Carbonic acid

Phosphoric acid

Hydrotelluric acid

Nomenclature Summary Flowchart

RAINBOW MATRIX GAME

Link on Chemistry Geek.com on Chemistry I page

http://chemistrygeek.com/rainbow

Use [ ] to represent subscripts since you can’t enter subscripts into the computer

So H2O would be H[2]O

And Al2(SO4)3 would be Al[2](SO[4])[3]

Additional Polyatomic Ions (you do not have to memorize these, but they are in the game!)

Borate = BO3 -3 ; Silicate = SiO4

-4 ; Manganate = MnO4

-2 (permanganate is -1)